M.Sc. Chemistry Question paper
Loyola College M.Sc. Chemistry April 2003 Structural Inorganic Chemistry Question Paper PDF Download
LOYOLA COLLEGE (AUTONOMOUS), CHENNAI-600 034.
M.Sc. DEGREE EXAMINATION – chemistry
first SEMESTER – APRIL 2003
CH 1802/CH 719 structural inorganic chemistry
08.04.2002
1.00 – 4.00 Max: 100 Marks
PART – A (10 ´ 2 = 20 Marks)
Answer the following
- Mention one example each for spinel and inverse spinel.
- Mention coordination numbers in fluorite and antifluorite structures.
- Suggest a technique to study the following
(a) hydrogen bonding in ice (b) bond length in diborane.
- ZnO acts as a n- type semiconductor.
- Predict the structure of B4 H10 applying Wades Rules.
- What is radius ratio? What is its significance?
- Taking H2 molecule as example show how molecular orbitals are obtained?
- How are n and p-type extrinsic semiconductors prepared?
- Explain van der Waal’s forces.
- What are gas hydrates and clathrates? Cite examples.
PART – B (8 ´ 5 = 40 Marks)
Answer any eight of the following
- Discuss and compare the structures of Wurtzite and Zinc blende.
- How are silicates prepared? Mention their applications.
- How are metallocarboranes prepared?
- Mention the advantages of single crystal X-ray diffraction analysis.
- Write a note on Schottky and Frenkel defects.
- How is structure factor derived for an array of atoms in a crystal lattice?
- What is Madelung constant? Calculate this constant for NaCl crystal
(first two terms only)
- How is lattice energy calculated using Born-Haber cycle?
- Discuss factors which influence hard/soft nature of cations.
- Construct MO diagram for NO molecule and explain its magnetic property and stability.
- Arrange the following molecules according to increasingbond angles.
Give reason(s) (i) CH4 (ii) CH2F2 (iii) CH2I2.
PART –C (4 ´10= 40 Marks)
Answer any four of the following
- How are phosphonitric compounds prepared?
Discuss the structure of P3 N3 Cl6.
- Discuss the following structures and draw silicate units:
(i) beryl (ii) talc (iii) quartz (iii) pyrosilicate (3+3+2+2)
- Discuss structures of spinels and inverse spinels taking Mn3 O4as typical examples.
- Explain Fajan’s Rules with suitable examples.
- Using band theory discuss conductance properties of (i) Mg (I)Hg (iii) I2 (3+3+4)
- Write an essay on non-equeous solvents and their applications.
Loyola College M.Sc. Chemistry April 2003 Science & Society Question Paper PDF Download
LOYOLA COLLEGE (AUTONOMOUS), CHENNAI-600 034.
M.Sc. DEGREE EXAMINATION – chemistry
second SEMESTER – APRIL 2003
CH 2803/CH 820 science and society
28.04.2002
1.00 – 4.00 Max: 100 Marks
PART – A (10 ´ 2 = 20 Marks)
Answer the following
- How do scientific results reach society for development?
02. Write notes on (i) transfer of technology and (ii) transformation of technology.
- How is acid rain caused?
- What is meant by equilibrium of ecology?
- Cite advantages and disadvantages in using robots.
- What is meant by drug abuse? Cite one specific example.
- Why do scientists make assumptions?
- What are the promises and perils in using genetic engineering?
- Explain the terms (i) information and (ii) disinformation
- Describe ‘cost effectiveness of scientific research’.
PART – B (4 ´ 10 = 40 Marks)
Answer any four of the following
- How does scientific development influence culture of a society?
- What are the reasons for environmental degradation?
- ‘Science is not against religious sentiments’ –
- What is industrialization of science? What is its significance?
- Discuss the role of scientists as bridge between industries and ecology.
- Why do some biological species vanish from world? Is this change desireable always?
PART – C (2 ´ 20 = 40 Marks)
Answer any TWO of the following.
- Write an essay on planning a research project and its successful completion.
- Make a comparitive study on scientific development in rural and urban areas.
- What are advantages, disadvantages and threats in using computers and internet for scientific research?
- Analyse pros and cons of non-conventional energy sources, with special
reference to nuclear energy and solar energy.
Loyola College M.Sc. Chemistry April 2003 General Chemistry For Maths & Physics Question Paper PDF Download
LOYOLA COLLEGE (AUTONOMOUS), CHENNAI-600 034.
M.Sc. DEGREE EXAMINATION – chemistry
fourth SEMESTER – APRIL 2003
CH 4200/CHE 200 general chemistry for maths & physics
22.04.2002
9.00 – 12.00 Max: 100 Marks
PART – A (10 ´ 2 = 20 Marks)
Answer ALL the questions.
- Define Lattice energy.
- State Kohlrausch’s law.
- Draw the structure of glucose.
- How does a – amino acid exist in acidic medium and alkaline medium?
- What is Bordeaux mixture? What is it used for?
- Mention two applications of radio isotopes in medicine.
- What are antipyretics? Give one example.
- What happens when anthracene is brominated?
- What are mordants?
- Acetic acid in benzene exists as a dimer –
PART – B (8 ´ 5 = 40 Marks)
Answer any EIGHT questions
- Write a note on carcinogenic hydrocarbon.
- How is congo red prepared?
- Explain the mode of action of sulpha drug.
- How is anthracene isolated from coal tar?
- How are the following prepared?
(i) Malachite green (ii) aspirin
- Derive Kirchoff’s equation
- Draw the conductometric titration curves for the following and explain.
(i) HCl vs NaOH (ii) CH3 COOH Vs NaOH
- Discuss the factors affecting enzyme catalysis.
- Write a note on photosynthesis.
- Explain the features of nuclear fission reaction.
- Explain the construction of calomel electrode. What is the electrode reaction?
PART – C (4 ´ 10 = 40 Marks)
Answer any FOUR questions
- Construct Born Haber cycle for NaCl(s). Mention the terms involved.
- a) Discuss the primary structure of proteins. (5)
- b) Write a note on herbicides (5)
- a) Explain the role of micro-nutrients in the growth of plants (5)
- b) What is the role of enzyme in enzyme catalysis? (5)
- How is the dissociation constant of acetic acid determined using conductivity measurement?
- a) How are lanthanides separated by ion-exchange method? (6)
- Physical properties of compounds are affected by H-bonding – Explain
with two examples. (4)
- a) What are chromophores and auxochromes? Give examples. (5)
- How are the following conversions effected?
(i)pyrrole to 2-nitro pyrrole. (ii) Pyrrole to Pyrolle-2-aldehyde (5)
Loyola College M.Sc. Chemistry April 2003 Advanced Coordination Chemistry Question Paper PDF Download
LOYOLA COLLEGE (AUTONOMOUS), CHENNAI-600 034.
M.Sc. DEGREE EXAMINATION – chemistry
fourth SEMESTER – APRIL 2003
CH 4950/CH 1054 ADVANCED COORDINATION chemistry
23.04.2002
1.00 – 4.00 Max: 100 Marks
part – A (10 ´ 2 = 20)
- What is slipped Sandwich? Cite an example.
- Define coordination template effect. Cite a dinuclear complex synthesized by
the method.
- Justify the formation of coordination compounds of different geometries by d-
block metal ion with the help of angular overlap model.
- What is tetragonal splitting parameter? How is it evaluated?
- Differentiate CE and EC mechanisms.
- Give the structure of (a) Potassium ethylxanthate
(b) Dipheylphosphinoethane (dppe).
- How are he optical isomers of [Co (NH3)4 Cl2]+ distinguished?
- [NiCl4]2- has a magnetic moment of 2.84 B.M. Predict the geometry with hybridization of the metal atom.
- How are the complexes [Cr(NH3]4 Cl2]Cl and [Cr(NH3)3Cl3] distinguished by NQR spectroscopy?
- What role is played by cisplatin in the cancer therapy?
PART- B (8 ´ 5 = 40 Marks)
- Explain the principles of angular overlap model.
- What are compartmental ligands? Explain the different methods of syntheizing compartmental ligands and their polynuclear complexes.
- Explain the electronic spectral features of high-spin octahedral and tetrahedral complexes.
- Give an account of spectroelectrochemical techniques in studying electrogenerated species.
- Explain the principle of AC polarography. How is this technique useful to study the reversible redox couples?
- Explain with an example the experimental method of studying static dynamic Jahn-Teller effect.
- Explain that the isomer shift value of [Fe (CN)6]4– is more negative than that of
[Fe (H2O)6]2+ . D EQ of the former is zero and the later has a D EQ value of 3.3 mm s-1.
- Suggest a method of synthesis for
(a) [Co (NH3)6]Cl3 from CoCl2.6H2O (2)
(b) Cis and trans – [Pt(NH3)2Cl2] (1 ½ + 1 ½)
- Discuss the different sampling methods used in EPR spectroscopy. Bring out their advantages.
- How do the quantum yields vary in a photoanation reactions? Discuss with a suitable example.
- Discuss the coordination around iron in cytochrome and the role played by it in the biological processes.
- How is N(1s) photoelectron spectrum useful in the study of [Co(NH3)5 N3](NO3)2
PART – C (4 ´10 = 40 Marks)
- (a) Derive the Marcus-Hush equation for electron transfer.
- Explain how do the crystal field effect influence the rate of electron
transfer reactions.
- (a) Explain the electronic spectral features of low -spin d6 metal ion and
the method of computing Dqxy and Dqz values.
- How is spin crossover studied experimentally?
- Give an account of NMR spectra of paramagnetic compounds.
- Discuss the role played by the metal atoms in the Nitrogen fixation. Write a note
on biomimic coordination. cluster complexes of nitrogenase.
- (a) Explain the Mossbauer spectrum of FeF3 recorded at 4K. (5)
- Describe Krammer’s degeneracy choosing an example.
- (a) Discuss in detail the EPR spectrum of [Cu (salimine)2] along with the
hyperfine splitting by the ligand. (7)
(b) How does Cr(CO)6 undergo photochemical decomposition? (3)
Loyola College M.Sc. Chemistry Nov 2003 Thermodynamics & Statistical Mechanics Question Paper PDF Download
LOYOLA COLLEGE (AUTONOMOUS), CHENNAI –600 034
M.Sc., DEGREE EXAMINATION – CHEMISTRY
SECOND SEMESTER – NOVEMBER 2003
CH-2800/815 – THERMODYNAMICS & STATISTICAL MECHANICS
28-10-2003 Max:100 marks
1.00 – 4.00
PART – A (10×2=20 marks)
Answer ALL questions.
- If V = for 1mole of an ideal gas show that dV is a complete differential.
- Kp for the reaction at 500oC is 3.99×10-3 atm-1 Calculate DGo for the reaction.
- Show that .
- What is chemical potential? Is it extensive or intensive?
- How many components are present in a system in which NH4Cl (s) undergoes thermal decomposition?
- Calculate the number of ways of distributing 20 identical objects with the arrangement 1, 0, 3, 5, 10, 1.’
- What is the significance of partition function?
- What is the residual molar entropy of CO at T = O?
- Identify the systems for which it is essential to include a factor of on going from molar partition function to molecular partition function a) a sample of CO2 (g) b) water vapour.
- Calculate the ratio of the translation partition functions of D2 and H2 at the same temperature and pressure.
PART – B (8×5=40 marks)
Answer any EIGHT questions.
- Derive expressions for isothermal reversible expansion of 1 mol of Vander Waal’s gas for a) W b) D
- DS of a solid in cal/k/mole is given by the equation Cp = 6.2 + 1.3 x 10-3T in the temperature range 27oC to 600o Calculate DS when 1 mole of this metal is heated from 300 k to 600 k.
- Derive any two Maxwell equations.
- The volume of an aqueous soltuon of NaCl at 25oC was measured in series of molalities (m) and it was found that the volume fitted the expression
V (CC) = 1003 + 16.62m + 1.77 m3/2 + 0.km2 where V is the volume of a solution of molality 1. Calculate the partial molar volume of a the components in a solution of molality 0.1.
- 325 g of N2O4 when heated was found to occupy a volume of 500 ml at 45oC and at 800 mm Hg pressure Calculate i) Kp ii) pressure at which the degree of dissociation is 50%.
- Explain how partition functions can be separated.
- Calculate the standard molar entropy of Xenon gas at 100 K.
- Calculate the electronic partition function of a Tellurium atom at 500 K using the following data.
Term Degeneracy Wave number (cm-1)
Ground 5 0
1 1 4707
2 3 4751
3 5 10559
- Explain how the absolute entropy of a gas at 25oC can be determined using third law of thermodynamics.
- Compare Maxwell – Bolltzmann, Fermi – Dirac and Bose – Einstein statistical distributions.
- Calculate the molecular rotational partition function for N2 (g) at 27o
(I = 13.9 x 10-47 kgm-2).
- Derive an expression for transnational partition function.
PART – C (4×10=40 marks)
Answer any FOUR questions.
- a) Derive Gibbs – Duhem equation.
- b) Show that for 1 mole of a van der waal’s gas.
- a) Explain how activity coefficient of an electrolyte be determined using EMF data.
- b) Derive thermodynamically phase rule equation.
- a) The virial equation of state for N2(g) at OoC is
PV = RT – 1.051 x10-2 P + 8.63 x 10-5 P2 + ….
Where P is in atm; V is in litres. Find the fugacity of N2 at OoC and 100 atm.
pressure.
- b) Deduce the expression for the variation of chemical potential with i) temperature ii)
pressure.
- State the postulates of Maxwell – Boltzmann statistics and hence derive an expression for the most probable distribution.
- Compare Einstein’s theory of heat capacity of solids with Debye’s theory.
- a) Explain how equilibrium constant of a reaction be obtained using statistical mechanics.
- b) Explain transition state theory using statistical concepts.
- a) Derive the relation
E = .
- b) Calculate the vibrational contribution to the entropy of Cl2 at 500K if the wave
number of the vibration is 560 cm-1.
Loyola College M.Sc. Chemistry Nov 2003 Electrochemistry Question Paper PDF Download
LOYOLA COLLEGE (AUTONOMOUS), CHENNAI –600 034
M.Sc., DEGREE EXAMINATION – CHEMISTRY
FOURTH SEMESTER – NOVEMBER 2003
CH – 4803/1020 – ELECTRO CHEMISTRY
01-11-2003 Max:100 marks
1.00 – 4.00
PART – A (10X2=20 marks)
Answer ALL questions.
- The limiting molar conductance of OHis highest among the anions – Explain.
- Calculate the ionic strength of a mixture containing 20 mL of 0.1M lanthanum sulphate, 30 mL of 0.5 M magnesium nitrate and 50 mL of water.
- In case of alkali halides the deviation from Debye Huckel Onsager equation is more marked as the atomic weight increases – Explain.
- Calculate the limiting molar conductance of lanthanum ion if its mobility is 7.21 x 10-8 m2 V-1 S-1.
- Write Lippmann’s first equation and mention its importance.
- Draw the plot of current density vs applied potential for an electrolytic solution and hence indicate the discharge potential of an ion.
- Mention the electrical properties that influence the rate of an electrochemical reaction.
- Bring out the differences between symmetry factor and transfer coefficient.
- What do you mean by non-polarisable electrode?
- Define exchange current density.
PART – B (8X5=40 marks)
Answer any EIGHT questions.
- Calculate the instability constant of the complex formed in the reaction
Cu+2 + 4 NH3 [Cu (NH3)4]+2
Given Cu+2 +2 Cu(s) Eo = 0.337 V
[Cu (NH3)4]2+ + 2 Cu(s) + 4 NH3 Eo = -0.12 V.
- 2 M lead nitrate solution freezes at -0.05oC. Calculate its dissociation constant. Cryoscopic constant of water is 1.86 kg K mol-1.
- The dissociation constant of chloroacetic acid is 1 x 10-4. Will the degree of dissociation increase or decrease if 0.1 M KCl is added to 0.1 M chloro acetic acid?
- Write notes on electro kinetic phenomena.
- Discuss electrocapillary phenomena.
- How is the limiting molar conductance of acetic acid determined using Debye Huckel Onsager – equation?
- Compare the rates of reduction of Ag+, at over voltages -0.1 and +0.1 V, which has a symmetry factor, = 0.5.
- Explain any one experimental method of determining the exchange current density.
- State Butler – volmer equation for one electron process. Derive Nernst equation from it.
- Determine the order of the reaction 2 H3O+ + 2e 2 H2O + H2 in acidic medium.
- Derive Tafel equation for cathodic process.
- Define half wave potential. Show that it is a constant characteristic of the electro active species.
PART – C (4X10=40 marks)
Answer any FOUR questions.
- State the postulates of Debye Huckel theory and derive an expression for Debye Huckel length.
- Derive Debye Huckel limiting law. How is it verified? Mention its applications.
- What are the features of Helmholtz Perrin model? What are its limitations? How are these overcome in Stern’s model?
- a) Derive the Butler – Volmer equation for a multistep electrochemical reaction.
- b) Explain the condition under which the above equation reduces to simpler Butler –
Volmer equation.
- a) A cathodic potential of 3V is applied to Cu2+ and Na+ solutions separately. Calculate
the over potential of the two electrodes.
- b) Explain any three applications of polarography.
- a) Obtain an expression for limiting current on the basis of concentration polarization.
- b) Write a note on
- Cyclic voltametry
- Amperometric titrations
Loyola College M.Sc. Chemistry Nov 2003 Analytical Chemistry Question Paper PDF Download
LOYOLA COLLEGE (AUTONOMOUS), CHENNAI –600 034
M.Sc., DEGREE EXAMINATION – CHEMISTRY
THIRD SEMESTER – NOVEMBER 2003
CH – 3805/924 – ANALYTICAL CHEMISTRY
10-11-2003 Max:100 marks
1.00 – 4.00
PART – A
Answer ALL the questions. (10×2=20 marks)
- Explain constant error with an example.
- Ce+4 + Ce+3 Eo = 1.44 V
Sn+4 + 2 Se+2 Eo = 0.15 V
Compute the equivalence point potential for the above system.
- Explain replacement titration with an example.
- Mention the factors which affect the pM value at the equivalence point.
- Calculate the equivalence point pH when 20.00 mL of 0.1000 M CH3 COOH is titrated against 0.2000M NaOH (Ka for CH3 COOH 1 x 10-5)
- How will you estimate phenol coulometrically?
- Bring out the difference between Voltametric and potentiometric methods of analysis.
- Explain the role of supporting electrolyte in polarography.
- Explain why photoemission occurs at higher wave length than absorption.
- What do you mean by carrier gas in GC? Give an example.
PART – B
Answer any EIGHT questions. (8×5=40 marks)
- Calculate the concentration of Ce+4 and Fe+2 in the mixture containing 20.00 mL of
0.100 N Fe+2 and 40.00 mL of 0.0500 N Ce+4 in acidic medium. E= 1.44 V and E= 0.77 V.
- What are metallochromic indicators? Give an example with the structure. What are its characteristics?
- How is an outlier rejected using Q-test.
- Calculate the value of pZn in the mixture containing (I) 50.00 mL of 0.015 M Zn+2 and 30.00 mL of 0.025 M EDTA (ii) 50.00 mL of 0.025 M Zn+2 and 50.00mL of 0.050 M EDTA, both at pH 10.
- Write a note on Von Weimarn’s theory.
- Calculate the pH at which Mg(OH)2 begins to precipitate from 0.1000 Mg(NO3)2.
Ksp of Mg(OH)2 = 1×10-11.
- What is DTGA? Compare it with DSC.
- What do you men by steam distillation? What are the condition for a compound to be steam distilled?
- A 0.5 millimolar solution of a divalent metal ion solution has diffusion current of 4 m The dropping rate of Hg was 24 drops½min. The mass of 40 drops was found to be 15 mg. Calculate the diffusion coefficient of the ion.
- a) Explain the mechanism phosphorescence.
- b) Explain the effect of the following on the intensity of fluorescence. (i) solvent (ii) pH
(iii) Dissolved oxygen.
- Interpret the DTGA pattern of an inorganic compound with a suitable example.
- a) Explain the principle of solvent extraction.
- b) Obtain an expression for the amount of substance extracted at the end of nth extraction
using small volume of the extracting solvent each time.
PART – C
Answer any FOUR questions. (4×10=40 marks)
- Give a critical account of acid base titrations in non-aqueous solvents.
- a) A 1.0000g sample containing Na2C2O4 requires 00 mL of 0.0200 M KMnO4 the for
oxidation in acid medium. Calculate the percentage of Na2C2O4 in the sample and
express it scientifically.
- b) A blood sample is sent to two different laboratories to be analyzed for cholesterol. The
results obtained for the concentration (mg/dL) were:
Laboratory I Laboratory II
= 243 = 258
s1 = 13 s2 = 15
n1 = 11 n2 = 11
- Are the standard deviations significantly different at the 95% level?
- Are the two means significantly different at the 95% level?
F value at 95% probability level for the above set corresponds to 2.98. Students ‘t’
value at 95% probability level is 2.26.
- a) What are the advantages and disadvantages of organic reagents in gravimetry?
- b) A 0.3500 g sample containing KCl and KI gives a precipitate of AgCl and AgI that
weighs 0.2720 g. A 0.5250 g sample of the same material is titrated with 0.1020 M
AgNO3 requiring 25.80 mL. Calculate the percentages of KCl and KI in the sample.
- a) What is the difference between electro-gravimetric method and Coulometric method.
- b) Explain the analytical method involved in the estimation Cu+2 by
- Electro gravimetric method
- Polarographic method
- a) Give the schematic representation of different types of variation of applied potential as
a function of time adopted in voltametry
- b) Write a note on cyclic voltametry.
- a) Draw the absorption, fluorescence and phosphorescence spectrum of a typical
compound.
- b) Give the schematic diagram of a spectroflurometer and explain the components.
Loyola College M.Sc. Chemistry April 2006 Organics Substitution,Addition & Elimination Rxn Question Paper PDF Download
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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034
M.Sc. DEGREE EXAMINATION – CHEMISTRY
SECOND SEMESTER – APRIL 2006
CH 2808 – ORGANIC SUBSTITUTION, ADDITION & ELIMINATION RXN
Date & Time : 19-04-2006/FORENOON Dept. No. Max. : 100 Marks
Part-A
Answer ALL questions. (10 ´ 2 = 20)
- Predict the product with mechanism
- What is ipso attack? Give the possible mechanism for ipso attack.
- What are stable, persistent and inert free radicals? Give example.
- Predict the product of the reaction of dihydropyran with primary alcohols in the presence of acids with mechanism.
- Predict the product.
- How would you explain that trans-2-acetoxycyclohexyl brosylate with acetate in glacial acetic acid gives only trans diacetate?
- Explain Grunwald-Winstein equation.
- Which of the following is more nucleophilic? Why? Benzene or mesitylene; Phenoxide or p-nitrophenoxide
- Explain Hofmann’s rule in elimination reactions with a suitable example.
- What are ambident nucleophiles? Give an example.
PART B
Answer any EIGHT questions (8 ´ 5 = 40)
- Give the mechanism of the following:
- a) Wohl-Ziegler bromination b)Wittig rearrangement.
- a) Predict the product with mechanism
- b) Explain Bartons reaction.
- Give the mechanism of oxymercuration reaction. Also give the evidences for the free radical mechanism for the cleavage of Hg.
- Predict the product with mechanism and evidence.
- Define isoinversion. Explain using a suitable example.
- Using suitable resonance-stabilizing structures explain why halogens are deactivators but o, p-directors.
- How would you show that the transition state in SN2 reaction must be linear?
- Threo DL pair of 3-bromo-2-butanol with HBr gave DL-2,3-dibromobutane while the erythro pair gave meso isomer. Explain.
- Explain ion-pair mechaism. What are its evidences?
- ‘Basic hydrolysis of a-bromopropionate ion with concentrated base gives a product with inverted configuration but with dilute base, retention product is formed’. Explain.
- What happens when the following are subjected to pyrolysis?
(i) 2-acetoxybutane (ii) Xanthate from isobutyl alcohol - Solvolysis in acetone-water at 85°C of syn-7-p-anisyl-anti-7-norborn-2-enyl p-nitrobenzoate was only 2.5 times faster than that of the saturated compound’.
PART C
Answer any FOUR questions (4 ´ 10 = 40)
- How are the following synthesized from benezene?
a) m-nitroacetophenone b) p-chlorobenzoic acid
c)p-propylbenzen sulphonic acid d) m-bromopropylebenzene. - a) How are the following conversions effected?
- b) Propose a synthesis for the following compounds using Robinson annulations.
- a) Give the mechanism of free radical substitution at an aromatic substrate. Substantiate it with suitable evidences.
b) 2,3-dimethylbutane gives different ratio of products in aliphatic and aromatic solvents. Why? - a) Endo-anti-tricyclo[3.2.1.02-4]octan-8-yl-p-nitrobenzoate is solvolysed about 1014times faster than p-niotro isomer containing C=C’. Explain.
- b) How would you show by reactions the mechanistic border line region between SN1 and SN2 reactions?
- a) Solvolysis of L-threo-3-phenyl-2-butyltosylate in acetic acid gives threo product in major amount’. Explain.
- b) What is ‘Product spread’ in elimination reactions? Explain with suitable examples.
- a) Explain Bucherer reaction with mechanism.
- b) Expalin the following:
(i) Acetolysis of both 4-methoxy-1-pentylbrosylate and 5-methoxy-2-pentylbrosylate give the same mixture of products.
- Both erythro- and threo-1-acetoxy-2-deutero-1,2diphenylethane on pyrolysis give the same product.